The Pressure Of 4 Liters Of Oxygen Gas Is 3 Pa

The Pressure Of 4 Liters Of Oxygen Gas Is 000003 Pa If We Change The

The Pressure Of 4 Liters Of Oxygen Gas Is 000003 Pa If We Change The The pressure of 4 liters of oxygen gas is 0.00003 Pa. If we change the volume to 1.5 liters, what will the resulting pressure be? a.0008 Pa b.00003 Pa c.00008 Pa d. Pa The temperature of 18 liters of hydrogen gas is 373 K. If we change the temperature to 273 K, what will the resulting volume be? a.24.6 L b.13.2 L c.12.72 L d.12.3 L Air in a certain container has a pressure of 0.00025 Pa at a temperature of 312 K. If we change the temperature to 240 K, what will be the pressure? a.192 Pa b.0008 Pa c.000187 Pa d.000192 Pa

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The series of problems presented involve the application of fundamental gas laws—Boyle’s Law, Charles’s Law, and Gay-Lussac’s Law—each describing relationships between temperature, pressure, and volume of gases under varying conditions. These laws are essential components of the ideal gas law, PV=nRT, which encapsulates the behavior of ideal gases and allows us to predict the changes in pressure, volume, or temperature when one of these variables is altered, assuming the amount of gas remains constant.

Boyle’s Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature (P∝1/V), is used to determine the new pressure when the volume changes. Conversely, Charles’s Law describes how the volume of a gas varies directly with temperature (V∝T) at constant pressure, and Gay-Lussac’s Law relates pressure directly to temperature (P∝T) at constant volume.

In the first scenario, the initial conditions specify a pressure of 0.00003 Pa in a volume of 4 liters. When the volume is decreased to 1.5 liters, the application of Boyle’s Law allows us to find the new pressure. The law is mathematically expressed as P1V1 = P2V2, which rearranged gives P2 = P1V1 / V2. Substituting the known values yields the new pressure.

The second problem involves the ideal gas law to predict the new volume after changing the temperature of a gas sample. Starting with 18 liters at 373 K, and cooling the gas to 273 K, Charles’s Law states V1/T1 = V2/T2, allowing us to calculate the final volume.

The third problem requires understanding the relationship between pressure and temperature, keeping volume constant, based on Gay-Lussac’s Law. Starting with an initial pressure at 312 K, the temperature drop to 240 K leads us to calculate the new pressure with P1/T1 = P2/T2.

These problems underscore the importance of understanding gas laws for predicting how gases respond to changes in their environment, which is fundamental in fields such as chemistry, physics, environmental science, and engineering. Mastery of these principles supports accurate modeling and analysis of real-world systems involving gases.

Applying Boyle’s Law:

P1V1 = P2V2

Initial parameters: P1 = 0.00003 Pa, V1 = 4 L, V2 = 1.5 L

P2 = (0.00003 Pa * 4 L) / 1.5 L = (0.00012 Pa·L) / 1.5 L = 0.00008 Pa

The answer is c. 0.00008 Pa.

Applying Charles’s Law:

V1/T1 = V2/T2

Initial parameters: V1 = 18 L, T1 = 373 K, T2 = 273 K

V2 = V1 T2 / T1 = 18 L 273 K / 373 K ≈ 13.2 L

The answer is b. 13.2 L.

Applying Gay-Lussac’s Law:

P1/T1 = P2/T2

Initial parameters: P1 = 0.00025 Pa, T1 = 312 K, T2 = 240 K

P2 = P1 T2 / T1 = 0.00025 Pa 240 K / 312 K ≈ 0.000192 Pa

The answer is d. 0.000192 Pa.

These calculations demonstrate how fundamental gas laws allow us to predict the behavior of gases under different conditions accurately. This understanding is critical in designing chemical processes, environmental controls, and understanding atmospheric phenomena.

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